Thorium
Thorium is a chemical element; it has symbol Th and atomic number 90. Thorium is a weakly radioactive light silver metal which tarnishes olive grey when it is exposed to air, forming thorium dioxide; it is moderately soft, malleable, and has a high melting point. Thorium is an electropositive actinide whose chemistry is dominated by the +4 oxidation state; it is quite reactive and can ignite in air when finely divided.
All known thorium isotopes are unstable. The most stable isotope, 232Th, has a half-life of 14.0 billion years, or about the age of the universe; it decays very slowly via alpha decay, starting a decay chain named the thorium series that ends at stable 208Pb. On Earth, thorium and uranium are the only elements with no stable or nearly-stable isotopes that still occur naturally in large quantities as primordial elements. Thorium is estimated to be over three times as abundant as uranium in the Earth's crust, and is chiefly refined from monazite sands as a by-product of extracting rare-earth elements.
Thorium was discovered in 1828 by the Swedish chemist Jöns Jacob Berzelius during his analysis of a new mineral found by Morten Thrane Esmark in Norway on Lovoya island near Brevik in the Langesund fjord. He named it after Thor, the Norse god of thunder and war. Its first applications were developed in the late 19th century. Thorium's radioactivity was widely acknowledged during the first decades of the 20th century. In the second half of the 20th century, thorium was replaced in many uses due to concerns about its radioactive properties.
Thorium is still used as an alloying element in TIG welding electrodes but is slowly being replaced in the field with different compositions. It was also material in high-end optics and scientific instrumentation, used in some broadcast vacuum tubes, and as the light source in gas mantles, but these uses have become marginal. It has been suggested as a replacement for uranium as nuclear fuel in nuclear reactors, and several thorium reactors have been built. Thorium is also used in strengthening magnesium, coating tungsten wire in electrical and welding equipment, controlling the grain size of tungsten in electric lamps, high-temperature crucibles, and glasses including camera and scientific instrument lenses. Other uses for thorium include heat-resistant ceramics, aircraft engines, and in light bulbs. Ocean science has used 231Pa/230Th isotope ratios to understand the ancient ocean.
Bulk properties
Thorium is a moderately soft, paramagnetic, bright silvery radioactive actinide metal that can be bent or shaped. In the periodic table, it lies to the right of actinium, to the left of protactinium, and below cerium. Pure thorium is very ductile and, as normal for metals, can be cold-rolled, swaged, and drawn. At room temperature, thorium metal has a face-centred cubic crystal structure; it has two other forms, one at high temperature and one at high pressure.Thorium metal has a bulk modulus of 54 GPa, about the same as tin's. Aluminium's is 75.2 GPa; copper's is 137.8 GPa; and mild steel's is 160–169 GPa. Thorium is about as hard as soft steel, so when heated it can be rolled into sheets and pulled into wire.
Thorium is nearly half as dense as uranium and plutonium and is harder than both. Thorium has a magnetic susceptibility of 0.412 × 4π × at room temperature. This susceptibility is mostly temperature-independent, however impurities and dopants can affect this value. It becomes superconductive below 1.4 K. Thorium's melting point of 1750 °C is above both those of actinium and protactinium. At the start of period 7, from francium to thorium, the melting points of the elements increase, because the number of delocalised electrons each atom contributes increases from one in francium to four in thorium, leading to greater attraction between these electrons and the metal ions as their charge increases from one to four. After thorium, there is a new downward trend in melting points from thorium to plutonium, where the number of f-electrons increases from about 0.4 to about 6: this trend is due to the increasing hybridisation of the 5f and 6d orbitals and the formation of directional bonds resulting in more complex crystal structures and weakened metallic bonding. Among the actinides up to californium, which can be studied in at least milligram quantities, thorium has the highest melting and boiling points and second-lowest density; only actinium is lighter. Thorium's boiling point of 4788 °C is the fifth-highest among all the elements with known boiling points.
The properties of thorium vary widely depending on the degree of impurities in the sample. The major impurity is usually thorium dioxide ; even the purest thorium specimens usually contain about a tenth of a per cent of the dioxide. Experimental measurements of its density give values between 11.5 and 11.66 g/cm3: these are slightly lower than the theoretically expected value of 11.7 g/cm3 calculated from thorium's lattice parameters, perhaps due to microscopic voids forming in the metal when it is cast. These values lie between those of its neighbours actinium and protactinium, part of a trend across the early actinides.
Thorium can form alloys with many other metals. Addition of small proportions of thorium improves the mechanical strength of magnesium, and thorium–aluminium alloys have been considered as a way to store thorium in proposed future thorium nuclear reactors. Thorium forms eutectic mixtures with chromium and uranium, and it is completely miscible in both solid and liquid states with its lighter congener cerium.
Isotopes
There are seven naturally occurring isotopes of thorium but none are stable.232Th is the only isotope of thorium occurring in quantity in nature; its half-life is 14.0 billion years, about three times the age of the Earth, and slightly longer than the age of the universe, and longest of all nuclides heavier than bismuth. Its stability is attributed to its closed nuclear subshell with 142 neutrons. Thorium has a characteristic terrestrial isotopic composition, with atomic weight. It is one of only four radioactive elements that occur in large enough quantities on Earth for a standard atomic weight to be determined.
Thorium nuclei are susceptible to alpha decay because the strong nuclear force cannot overcome the electromagnetic repulsion between their protons. The alpha decay of 232Th initiates the 4n decay chain, or thorium series, which includes isotopes with a mass number divisible by 4. This chain of consecutive alpha and beta decays begins with the decay of 232Th to 228Ra and terminates at 208Pb. Any sample of thorium or its compounds contains traces of these daughters, which are isotopes of thallium, lead, bismuth, polonium, radon, radium, and actinium. Natural thorium samples can be chemically purified to extract useful daughter nuclides, such as 212Pb, which is used in nuclear medicine for cancer therapy. 227Th can also be used in cancer treatments such as targeted alpha therapies. 232Th also very occasionally undergoes spontaneous fission rather than alpha decay, but at a much lower rate than uranium-238 and all natural fission products and evidence come predominantly from it. Its partial half-life for this process is very long at over 1021 years.
In total, 32 radioisotopes have been characterised, which range in mass number from 207 to 238. After 232Th, the most stable of them are 230Th, 229Th, 228Th, 234Th, and 227Th. All of these isotopes occur in nature as trace radioisotopes due to their presence in the decay chains of 232Th, 235U, 238U, and 237Np: the last of these is long extinct in nature due to its short half-life, but is continually produced in minute traces from neutron capture in uranium ores. 233Th occurs naturally as the result of neutron activation of natural 232Th.
In deep seawaters the isotope 230Th constitutes up to of total thorium. This is because its parent uranium is generally soluble in the ocean, but 232Th is nearly insoluble and is precipitated; thus the isotopes continually produced from uranium is relatively enriched. For this reason International Union of Pure and Applied Chemistry reclassified thorium as a binuclidic element in 2013; it had formerly been considered a mononuclidic element.
Thorium has a nuclear isomer, 229mTh, having the lowest known excitation energy of any isomer, measured to be. This is so low that when it undergoes isomeric transition, the emitted gamma radiation is in the ultraviolet range. The nuclear transition from 229Th to 229mTh is being investigated for a nuclear clock.
Different isotopes of thorium are chemically identical, but have slightly differing physical properties: for example, the densities of pure 228Th, 229Th, 230Th, and 232Th are respectively expected to be 11.5, 11.6, 11.6, and 11.7 g/cm3. The isotope 229Th is fissionable and the bare critical mass of estimated at 2839 kg, although with steel reflectors this value would drop to 994 kg. 232Th is not fissionable, but it is fertile as it can be converted to fissile 233U by neutron capture and subsequent beta decay.